Kinetics Flashcards
1
Q
Requirements for a reaction to occur
A
- collision
- sufficient energy
- correct orientation
2
Q
Effect of increased surface area (smaller solid size) on rate of reaction
A
- more solid reactant is exposed
- more collisions can occur at once
- rate of reaction increases
3
Q
Effect of temperature increase on rate of reaction
A
- particles move around more quickly
- more collisions occur
- particles have higher energy
- more collisions result in reaction
- rate of reaction increases
4
Q
Effect of increased pressure on rate of reaction
A
- more collisions occur with the gas reactant
- rate of reaction increases
5
Q
Effect of increased concentration on rate of reaction
A
- more aqueous reactant per unit volume
- more collisions occur
- rate of reaction increases
6
Q
Effect of temperature increase on a boltzmann distribution
A
- area under the curve stays the same
- peak moves down to the right
- more particles are above reaction energy
7
Q
How a catalyst increases rate of reaction
A
- provides alternative reaction path with lower activation energy
- more collisions result in reaction
- rate of reaction increases
8
Q
Economic advantages of catalysts
A
- increased rate of reaction so greater yield of products
- reactions can occur at lower temperature, so lower energy costs and equipment requirements
9
Q
Why are solid catalysts used for gas reactions
A
Gas molecules are adsorbed onto the solid, making them more likely to collide and react
10
Q
Effect of a catalyst on a boltzmann distribution
A
- shape of the curve stays the same
- activation energy is lower
- more particles have enough energy to react
